Iron(III) oxide and hydrogen react to form iron and water, like this: Fe_2O_3(s) + 3H_2(g) rightarrow 2Fe(s) + 3H_2O(g) At a certain temperature, a chemist finds that a 5.4 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, iron, and water at equilibrium has the following composition: Calculate the value of the equilibrium constant K_c for this reaction. Round your answer to 2 significant digits.

Complete Question

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The equilibrium constant is  

Explanation:

      From  the question we are told that

              The chemical reaction equation is

The voume of the misture is    

  The molar mass of   is a constant with value of  

    The molar mass of      is a constant with value of  

    The molar mass of      is a constant with value of  

Generally the number of moles  is mathematically given as

    For  

     For  

       For  

Generally the concentration of a compound  is mathematicallyrepresented  as

      For  

       For  

      For  

  The equilibrium constant  is mathematically represented as

  Considering

            And      

At  equilibrium the

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.